Specific Heat (2 substance) Problems

A piece of unknown metal with mass 17.19 g is heated to an initial temperature of 92.50 °C and dropped into 25.00 g of water (with an initial temperature of 24.50 °C) in a calorimeter. The final temperature of the system is 30.05°C. What is the specific heat of the metal?

0.5407 J/g°C

A 140.0-g sample of water at 25.0°C is mixed with 100.0 g of a certain metal at 100.0°C. After thermal equilibrium is established, the (final) temperature of the mixture is 29.6°C. What is the specific heat of the metal, assuming it is constant over the temperature range concerned?

0.38 J/g°C

55.0g of a "mystery metal" is heated to 93°C in a hot water bath, and is then placed in a calorimeter containing 100.0 g of water at 25°C. The metal sits in the water until the temperature levels off at 29°C. At this point, both the metal and the water are at 29°C. The specific heat capacity of water is 4.184 J/g°C. Find the specific heat capacity of the metal.

0.475 J/g°C

84.0 g of a metal are heated to 99ºC in a hot water bath, and then placed in a coffee cup calorimeter containing 60.0 g of water at 32ºC. The final temperature in the calorimeter is 42ºC. What is the specific heat of the metal?

0.52 J/g°C

240 g of water (initially at 20°C) are mixed with an unknown mass of iron (initially at 500°C). When thermal equilibrium is reached, the system has a temperature of 42°C. Find the mass of the iron.

107.3 g

135 g of aluminum (initially at 400°oC) are mixed with an unknown mass of water (initially at 25°C). When thermal equilibrium is reached, the system has a temperature of 80°C. Find the mass of the water.

168.6 g

In the lab, an experimenter mixes 75.0 g of water (initially at 30°C) with 83.8 g of a solid metal (initially at 600°C). At thermal equilibrium, he measures a final temperature of 50.0°C. What metal did the experimenter probably use? Hint: look up some common specific heats of metals to help determine your answer.

tungsten

A sample of ice at -12°C is placed into 68 g of water at 85°C. If the final temperature of the system is 24°C, what was the mass of the ice?

37.8 g

The specific heat of aluminum is 0.90 J/gºC. 30.0 g of aluminum are heated in a hot water bath to 98ºC, and added to a calorimeter containing water at 25ºC. The final temperature in the calorimeter is 32ºC. What mass of water was in the calorimeter?

60.9 g

On a cold winter day, a steel metal fence post feels colder than a wooden fence post of identical size because

a) The specific heat capacity of steel is higher than the specific heat capacity of wood.

b) The specific heat capacity of steel is lower than the specific heat capacity of wood.

c) Steel has the ability to resist a temperature change better than wood.

d) The mass of steel is less than wood so it loses heat faster.

e) Two of the above statements are true.

b) The specific heat capacity of steel is lower than the specific heat capacity of wood.

If 26 g of water at 18°C are mixed with 49 g of water at 70°C, find the final temperature of the system.

52.0°C

If 84 g of water at 22°C are mixed with 150 g of ethanol at 88°C, find the final temperature of the system.

55.7°C

If 20 g of silver at 350°C are mixed with 200 g of water at 30°C, find the final temperature of the system.

31.8°C

A piece of rhodium with a mass of 24.50 g and an initial temperature of 96.00 °C was dropped into a calorimeter containing 30.08 g of distilled water. The final temperature of the metal and water in the calorimeter was 30.07 °C. What was the initial temperature of the water?

26.96 °C

A 322 g sample of lead (specific heat = 0.138 J/g°C) is placed into 264 g of water at 25°C. If the system's final temperature is 46°C, what was the initial temperature of the lead?

568°C